H CH 8 HOMEWORK
Assign oxidation numbers to the following:
+1 –1+2 -1 +4 –2 0+3 –2+5 -2
NaClMgBr2SO2AlNO2-1PO4-3
+1 +3 –2+1 –3+2 +5 –2+4 –1 +1 +7 –2-3 +1
Na3BO3Na3NCa(NO3)2CBr4KClO4NH4+1
- Distinguish between binary and ternary acids and give two examples of each.
Binary contain hydrogen and a nonmetal; ternary contain hydrogen and a polyatomic ion.
- What are monatomic ions?
A single atom with a charge.
- In naming and writing formulas, what determines the order in which the elements appear? Positive ions come first; elements are written from least electronegative to most electronegative with some exceptions.
- What are oxidation numbers?Number that show the distribution of electrons in a compound. These are NOT IONS!
Monatomic Ions:
O-2oxideSulfideS-2
Mg+2magnesium ionTin (II) ionSn+2
Fe+3Iron (III) ionBarium ionBa+2
N-3nitrideFluoride F-1
Ag+1silver ionCopper (I) ionCu+1
Binary Molecular:
N2F2dinitrogen difluorideDinitrogen MonoxideN2O
CI4carbon tetraiodidePhosphorus TrichloridePCl3
NO2nitrogen dioxidePentabromine DioxideBr5O2
P3O4triphosphorus tetraoxideSulfur MononitrideSN
SCl2sulfur dichlorideCarbon DisulfideCS2
Binary Ionic:
MgCl2magnesium chlorideNickel (II) ChlorideNiCl2
W2O3tungsten (III) oxideVanadium (III) PhosphideVP
ZnSzinc sulfideSilver SulfideAg2S
AlF3aluminum fluoridePotassium ChlorideKCl
Cd3P2cadmium phosphideCalcium SelenideCaSe
FeNiron (III) nitrideMolybdenum (VI) FluorideMoF6
Ferric nitride
Cs2 Scesium sulfideCadmium BromideCdBr2
Y2O3yttrium oxideManganese (II) NitrideMn3N2
SnI4tin (IV) iodideGold (I) OxideAu2O
Stannic iodide
Cu3P2copper (II) phosphideTitanium (IV) SulfideTiS2
Cupric phosphide
Polyatomic Ionic:
NaNO3sodium nitrateMagnesium BorateMg3(BO3)2
WPO4tungsten (III) phosphateTin (IV) SulfateSn(SO4)2
K2SO3potassium sulfiteCalcium BicarbonateCa(HCO3)2
Mg(C2H3O2)2magnesium acetateHydrogen PeroxideH2O2
Fe(BrO3)2Iron (II) bromateSodium AzideNaN3
Ferrous bromate
KMnO4potassium permanganateLead (II) TartratePbC4H4O6
ZnCr2O7zinc dichromateCopper (II) Ortho-Silicate
Cu2SiO4
Al2(CO3)3aluminum carbonateHydrogen CyanideHCN
Cd3[Fe(CN)6]2Iridium (VI) Hydroxide
cadmium ferricyanideIr(OH)6
AgClOsilver hypochloriteBarium NitrateBa(NO3)2
Acids:
HClhydrochloricacidSulfuric AcidH2SO4
HIO3 iodic acidHydrofluoric AcidHF
H2CO3carbonic acidsulfurous acidH2SO3
HBrhydrobromic acidOxalic AcidH2C2O4
Formula Writing:
potassium chlorate KClO3potassium chlorideKCl nickel (II) phosphide Ni3P2 stannic nitrite Sn(NO2)4 aluminum borate AlBO3 cobalt (III) sulfate Co2(SO4)3
cadmium sulfateCdSO4ammonium carbonate(NH4)2CO3
magnesium hydroxideMg(OH)2aluminum sulfiteAl2(SO3)3
sodium bromideNaBrsilver acetateAgC2H3O2
zinc nitrateZn(NO3)2sulfur dioxideSO2
phosphoric acidH3PO4ammonium chlorateNH4ClO3
zinc sulfideZnSpotassium nitrideK3N
gold (I) dichromateAu2Cr2O7lead (IV) phosphatePb3(PO4)4
lead (II) iodatePb(IO3)2calcium acetateCa(C2H3O2)2
cupric phosphateCu3(PO4)2lithium dichromateLi2Cr2O7
aluminum oxideAl2O3potassium oxideK2O
hydrobromic acidHBrammonium hydroxideNH4OH
barium hydroxideBa(OH)2magnesium borateMg3(BO3)2
carbon tetrachlorideCCl4sodium dichromateNa2Cr2O7
nitrogen dioxideNO2barium chlorateBa(ClO3)2
sodium bicarbonateNaHCO3carbonic acidH2CO3
calcium permanganateCa(MnO4)2citric acidH3C6H5O7
lithium nitriteLiNO2zinc iodateZn(IO3)2
cadmium perchlorateCd(ClO4)2barium chloriteBa(ClO2)2
manganese (II) oxideMnOmagnesium nitrideMg3N2
lithium borateLi3BO3cobalt (II) bisulfateCo(HSO4)2
hydroiodic acidHIferrous phosphateFe3(PO4)2
dinitrogen pentoxideN2O5carbon disulfideCS2
Naming:
Pb3(PO4)2lead (II) phosphateCoSO4cobalt (II) sulfate
CuSO4copper (II) sulfateCuSO3copper (II) sulfite
Pb(ClO3)4lead (IV) chlorateH2SO4sulfuric acid
Fe(N3)3iron (III) azideFe2(SO4)3iron (III) sulfate
Cr(OH)2 chromium (II) hydroxideKBrO3potassium bromate
Cd(IO3)2cadmium iodateFeCO3iron (II) carbonate
CaCr2O7calcium dichromateBa(NO3)2barium nitrate
KNO3potassium nitrateNH4C2H3O2ammonium acetate
Pb3N2lead (II) nitrideBa3P2barium phosphide
HClhydrochloric acidSO3sulfur trioxide
Mg(NO3)2magnesium nitrateHNO3nitric acid
Li2SO4lithium sulfate(NH4)2CO3ammonium carbonate
CuCrO4copper (II) chromateNaHCO3sodium bicarbonate
Ca(ClO2)2calcium chloriteBa(NO2)2barium nitrite
Ag2CrO4silver chromateSn3(PO4)2tin (II) phosphate
HC7H5O2benzoic acidCaH2calcium hydride
AuClO4gold (I) perchlorateMg(OH)2magnesium hydroxide
KHSO4potassium bisulphateSrCl2strontium chloride
MnSmanganese (II) sulfideAgNO3silver nitrate
P2O5 diphosphorous pentoxideFeHPO4iron (II) hydrogen phosphate
PCl5 phosphorous pentachlorideHC2H3O2acetic acid
H3PO4phosphoric acidN2Odinitrogen monoxide
Make a correction, if necessary, and then provide the name/formula.
CorrectionName/Formula
Ba3NO3Ba(NO3)2barium nitrate
KSO4K2SO4potassium sulfate
Mg3(PO4)2correctmagnesium phosphate
BaCr2O7correctbarium dichromate
NaC2H3O2correctsodium acetate
PbBr2correctlead (II) bromide
Ag2(CO3)2Ag2CO3silver carbonate
NaHCO3correctsodium bicarbonate
HSO4H2SO4sulfuric acid
NH4(NO2)2NH4NO2ammonium nitrite
Magnesium (II) hydroxidemagnesium hydroxideMg(OH)2
Dilithium oxidelithium oxideLi2O
Fluoric acidhydrofluoric acidHF
Calcium bicarbonatecorrectCa(HCO3)2
Pb(II)SO4PbSO4lead (II) sulfate
Practice Quiz:
Formula:Name:
1. silver___Ag____6. S-2sulfide
2. chromium (III) ion___Cr+3____7. I-1 iodide
3. yttrium ion___Y+3____8. Fe+3iron (III) ion
4. nitride___N-3____9. Ba+2barium ion
5. chlorine____Cl2___10. O-2oxide
Provide Formulas:
11. sodium sulfateNa2SO4
12. copper (I) oxideCu2O
13. potassium chloriteKClO2
14. calcium phosphateCa3(PO4)2
15. aluminum nitrideAlN
16. chromium (III) chlorideCrCl3
17. phosphorus trichloridePCl3
18. oxalic acidH2C2O4
19. barium phosphideBa3P2
20. gold (I) fluorideAuF
Provide Names:
21. P2O3 diphosphorous trioxide26. Ni(ClO3)2nickel (II) chlorate 22. SnCl2 tin (II) chloride 27. Pb3N4 lead (IV) nitride
23. ZnSzinc sulfide28. MgSO4magnesium sulfate
24. NaOHsodium hydroxide29. HBrhydrobromic acid
25. CuBr2copper (II) bromide30. K2Opotassium oxide
Calculate the Formula Mass of the following:
1. a. H2SO498 g/mol
b. Fe(C2H3O2)2 (SF)173.933 g/mol
c. CaSO4 2H2O172 g/mol
2. Determine the formula mass for the following. (SF)
H OH O
| | |
H—C—C—C—O—H
|
H89.0700 g/mol
3. Calculate the formula mass for acetylsalicylic acid:
180 g/mol9C/8H/4O
Mole Calculations:
1. Calculate the mass of 2.00 mols of sulfuric acid.
196 g
2. Calculate the number of moles in 60.00 g of potassium carbonate(SF).
FM = 138.2055 g/mol.4341 moles
3. Calculate the number of molecules in 2.00 g of carbon dioxide.
2.73 x 1022molecules
4. Find the number of grams in 7.2434 x 1024 ions of lithium ions.
84 g
5. 3.45 x 1023 “molecules” of barium phosphatewould contain how many atoms?
4.485 x 1024 atoms
Composition Stoichiometry:
1. 23 g of manganese (III) sulfate would contain how many grams of manganese?
6.4 g Mn
2. 77 g of phosphoric acid would contain how many mols of hydrogen?
2.36 mol H
3. 3.4 mols of zinc sulfite would contain how many grams of zinc?221 g Zn
4. 2.5 mols of calcium thiosulfate would contain how many mols of calcium?
2.5 moles Ca
5. 56.33 g of barium would be how many mols?.411 mol Ba
6. 657 g of sodium peroxide would contain how many mols of oxygen? (SF)
77.9783 g Na2O216.9 mol O
7. If a sample of iron (III) oxide contained 26 g of iron, what was the mass of the original sample? 37.14 g Fe2O3
8. 45 g of oxygen would be how many mols?
1.41 mols
9. 23 g of nitrogen dioxide would contain how many grams of oxygen? (SF)
16 g O
10. The average person exhales 500 mols of carbon dioxide in a day. How many grams of carbon would that be? 6000 g C
Calculate the Percent Composition of the following:
FM = 160 FM = 232
1a. Fe2O3b. Ag2O
70% Fe 30% O93% Ag 7% O
2. Determine the percent calcium in calcium phosphate.
38.71 %
3. For the compound sodium sulfate decahydrate, calculate the following:
a. %Nab. %Oc. %H2OFM = 322
14.3%70%56%
4. Calculate the mass of the metal in each of the following:
a. 50 g of MgS21.42 g Mg
b. 25 g of FeCO312.07g Fe
c. 200.00 g of aluminum oxide (SF)52.92506% Al
105.85 g Al
d. 10 g of copper (II) bromide
2.84 g
e. 50 g of lead (II) oxide which is 30% pure
13.93 g
f. 40 g of lead (IV) oxide which is 60% pure 20.79 g Pb
- The active ingredient in common household liquid bleach is the hypochlorite ion, ClO-
a) Determine the percent of active ingredient in sodium hypochlorite.69 %
b)If bleach contains a 5% solution of sodium hypochlorite by mass, calculate the
percentage of hypolchlorite ion in the bleach.3.45 %
- A sample of brass contains by mass 28.0% zinc and 72.0% copper. How many kilograms of brass could be produced from 6.00 kilograms of copper? 8.33 kg
7. A household detergent contains 35% sodium tripolyphosphate, Na5P8O10. This complex salt keeps the pH of the wash water slightly basic by buffering action. The tripolyphosphate can also form soluble complexes with hard water ions (Ca+2 and Mn+2) that would otherwise form insoluble precipitates with detergent molecules. Determine the percent of phosphorous in the detergent. 16.6 %
8. A bituminous coal sample had a mass of 20.0 g after complete drying. The coal’s sulfur was chemically converted to the precipitate barium sulfate. If the mass of the dry precipitate is 2.35 g, what was the percent sulfur in the dry coal?
1.61 %
Empirical and Molecular Formula Determination:
1. Calculate the empirical formula for the following compounds:
a. 63.1% Mn; 36.9% SMnS
b. 26.6% K; 35.4% Cr; 38.0% OK2Cr2O7
2. Find the empirical formula for a compound given that a 48.5g sample is found to contain 1.75g of carbon and 46.75g of bromine.
CBr4
3. The formula mass of a compound is 92g/mol. Analysis shows that there are .608g of nitrogen and 1.388g of oxygen. What is the molecular formula of the compound?
N2O4
4. Determine the molecular formula of a compound that has a formula mass of 220 and is 56.4% phosphorus and 43.7% oxygen.
P4O6
5. A 13.83 g sample of unknown decomposes when heated, giving CO2 (g) and 6.57g of solid MgO. What is the empirical formula for the compound?
MgCO3
6. 1.62g of CoCl2 xH2O gave a residue of .88g. Find the formula of the hydrate.
X = 6
7. 1.26g of CaSO4 xH2O gave a residue of .99g. Find the formula of the hydrate.
X = 2
8. What is the molecular formula of a hydrated sodium salt which has a formula mass of about 268g/mol and contains 46.9% water of hydration? An analysis reveals the following composition: Na 17.18%, P 11.57%, H 5.60%, O 65.70%
Na2HPO4 7 H2O
9. A hydrate magnesium compound has a formula mass of about 174 g/mol and contains 31.0% water of hydration. From the following analysis, calculate the molecular formula: Mg 13.90%, P 17.74%, H 4.01%, O 64.30%.
MgHPO4 3 H2O
Practice Quiz 1:
1. Assign oxidation numbers to the following:
+3 –2 +3 +6 -2
A. NO2-1B. Fe2(SO4)3
2. Determine the formula mass of #1B.
400 g/mol
3. 4 moles of carbon tetrachloride would contain how many moles of carbon?
4 mols C
4. If a sample of iron (III) oxide contained 2.5 moles of oxygen, then how many grams of iron would be in it?
93.33 g Fe
5. Find the percent composition of carbon tetrachloride.
8 % C 92 % Cl
6. Mass of crucible and contents before heating.21.54g
Mass of empty crucible.19.82g
Mass of crucible and contents after heating.20.94g
Find the percent water in the sample.34.88%
Practice Quiz 2:
1. What are the empirical and molecular formulas of a compound if 212.1g of the compound contains 42.4g of hydrogen and 169.7g of carbon. The formula mass of the compound is 30.0 g/mol.
CH3/ C2H6
2. What is the formula mass of lithium phosphate?
116 g/mol
3. How many grams of chromium are in 20g of chromium (II) chloride?
8.46 g Cr
4. 3.56 x 1023 molecules of carbon dioxide would be how many grams?
26.01 g CO2
5. 76g of copper (II) oxide would contain how many mols of copper and how many moles of oxygen? Why are these numbers the same? Would there be 38 g of each?
.96 mol Cu/.96 mol O/ Same ratio 1:1/ No atoms have different masses
Practice Quiz 3:
1. Assign oxidation numbers to the following:
+4 –2 +3 -2
A. IrS2B. C2O4-2
2. What is the formula mass of sodium tetraborate?
202 g/mol
3. 18.46g of copper (II) chloride would contain how many moles of chlorine?
.27 mol Cl
4. Find the percent composition of diphosphorous pentoxide.
43.66% P, 56.34% O
5. 11 moles of sulfuric acid would be how many grams?
1078 g H2SO4
6. Determine the molecular formula of a compound with a formula mass of 32 g/mol which is 87.5% nitrogen and 12.5% hydrogen. N2H4
1